Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

IGCSE Chemistry > Principles Of Chemistry > Flashcards

Principles Of Chemistry Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

Why do ionic compounds not have molecular formula?

A

Ionic compounds do not have molecular formula

Cos they DO NOT EXIST AS MOLECULES

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

The Periodic Table is arranged in order of

A

increasing atomic no.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

All elements in the same period have…

A

All elements in the same period have the same no. of ORBITAL SHELLS
(He is period 1!!)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Groups in vertical columns have..

A

Groups in vertical columns have
>same no. Of electrons in outer shell
>similar properties+reactions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

How many electrons does He have in its outer shell?

A

2e- unlike rest which have 8e-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

In the noble gases , does density increase up or down the group?

A

In the noble gases density INCREASES

DOWN THE GROUP

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

When a compound is heated and broken down into its elements— what name is given to this type of reaction.

A

Thermal decomposition

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Give the definition of ELECTROLYSIS

A

Electrolysis is a chemical change caused by passing electric current thru an ionic compound ( which is either molten or in solution)to set free the elements

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What must there be in order for something to conduct electricity ?

A

Charged particles.

Either e- or ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Describe structure of metals

A

A lattice structure of +ve ions surrounded by a sea of delocalised e-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Why do ionic compounds only conduct electricity when molten or in solution?

A

Because when ionic compounds are solid the ions are not free to move around, but when molten the IONS r free to move around

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What are ANIONS

A

-VE ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What are CATIONS

A

+VE ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Why do covalent compounds not conduct electricity?

A

Because they have NO CHARGED PARTICLES (all e- r held tightly in the atoms or in the bond)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What covalent compounds conduct when dissolved in water and why?

A

HCl gas + AMMONIA gas get ionised in water — therefore their e- are free to move around and conduct

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Define the term electrolyte

A

Electrolyte is a liquid or solution that undergoes electrolysis. Either molten/aq compounds OR solutions containing ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What are electrodes usually made of and why

A

Either graphite or platinum cos they’re CHEMICALLY INERT.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What’s an ANODE

A

+VE electrode

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What’s a CATHODE

A

-VE electrode

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What r molten compounds also called

A

A melt

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What electrode does reduction always occur at?

A

Reduction always occurs at the CATHODE (-VE electrode)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What electrode does oxidation always occur at?

A

Oxidation always occurs at the anode(+VE electrode)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Give the definition of IONIC BONDING

A

It’s the transfer of electrons from a metallic atom to a non- metallic atom

In doing so a +ve metal ion and -ve non metal ion is formed — the strong electrostatic attraction between the oppositely charged ions is an Ionic bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Name the force that holds the ions together in an ionic compound

A

Strong electrostatic attraction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Why can’t nitrate ions form ionic compounds with bromide ions

A

Because both nitrate ions and bromide ions are negatively charged
Ionic compounds can only be formed between positive + negative ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

What is the charge of a hydrogen ion

A

H+

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

What is the charge of a hydroxide ion

A

OH-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

What is the charge of a ammonium ion

A

NH4^+

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

What is the charge of a carbonate ion

A

Co3^ 2-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

What is the charge of a nitrate ion

A

NO3^-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

What is the charge of a sulfate ion

A

SO4^2-

32
Q

Why do compounds with giant ionic structures have high melting + boiling points

A

The electrostatic attraction between the oppositely charged ions is very strong and therefore a lot of energy is needed to overcome them … hence a high melting/boiling point

33
Q

What should one use to filter a solution

A

Filter paper

34
Q

What is an intermolecular force?

A

Force of attraction between covalent molecules — much weaker than the covalent bonds in a molecule

35
Q

Explain how the covalent bonds in the water molecule hold the hydrogen + oxygen atoms together

A

Strong electrostatic attraction between shared 2 electrons and nuclei (of hydrogen and oxygen)

36
Q

Why do covalent compounds not conduct electricity

A

Because they have no free electron + no ions

37
Q

What covalent compound conducts electricity and why

A

Graphite because it has delocalised electrons, as each carbon atom has only 3 bonds leaving 1 electron free

38
Q

Why do simple molecular structures with a high relative molecular mass have higher boiling points?

A

Because the intermolecular forces between molecules with a high relative molecular mass are STRONGER.

As there are more points along larger molecules for the intermolecular forces to act between— so more energy is needed to break the forces(hence higher boiling point)

39
Q

Why is C60 FULLERENE a poor conductor of electricity

A

Because although each carbon has one delocalised e-, the electron can’t move between molecules so it’s a poor conductor

40
Q

Why does diamond not conduct electricity

A

Because it has NO free electrons or ions

41
Q

Why does C60 Fullerene have a lower boiling point than diamond ?

A

Because it does not take as much energy to break the intermolecular forces of attraction in C60 FULLERENE compared to breaking the strong covalent bonds in diamond

42
Q

What forces is the simple molecular stucture C60 fullerene held together by

A

Intermolecular forces are the only forces that hold c60 Fullerene together

The layers can slide over each other, that’s why it’s a soft solid

43
Q

Explain why graphite conducts electricity

A

Because each carbon atom in graphite has only 3 covalent bonds, so 1 e- is left delocalised and free to move— conducting electricity

44
Q

Explain why graphite has a high melting point

A

Because it’s a giant covalent structure and the strong covalent bonds r hard to break

45
Q

Why do simple molecular structures have low melting boiling point/ (I.e. exist as liquids/gases or solids with low meliting points)

A

Because they have weak intermolecular forces, and not a lot of energy is required to break them

46
Q

What is an allotrope

A

Different forms of the same element

47
Q

Why is graphite soft and slippery

A

Although the covalent bonds are v strong, the attractions (aka INTERMOLECULAR FOCES) between the layers are much weaker and not a lot of energy is required to overcome them

48
Q

Diamond, graphite + C60 Fullerene are 3 ______ of carbon

A

Diamond, graphite + C60 Fullerene are 3 allotropes of carbon

49
Q

Is a high or low temperature required to turn carbon to diamond if it’s enthalpy value is +37

A

A high temperature cos the energy required to break the covalent bond is +ve value meaning it’s an endothermic reaction which absorbs heat

50
Q

The bonding in a hydrogen molecule is strong.

Explain why the boiling point of hydrogen is low

A

Because although the bonding in each hydrogen molecule is strong
The intermolecular forces between individual molecules is weak and therefore little energy is required to overcome them

51
Q

Explain how to atoms in a chlorine molecule are held together

A

The 2 atoms share electrons which hold them together in a covalent bond, which is the electrostatic attraction between the shared pair of electrons and the nuclei of both atoms

52
Q

What is an element

A

Substances that can’t be split into anything simpler by chemical means. CONTAIN ONLY 1 TYPE OF ATOM

53
Q

What is a compound

A

When 2 or more different elements chemically combine

54
Q

Why is sulfur yellow in colour and iron sulfide not?

A

Cos iron sulfide is a compound and sulfur is an element

The properties of a compound are often completely different to the properties of the original elements

(so a compound of sulfur is not yellow like the element itself)

55
Q

Why are compounds hard to separate and mixtures not?

A

Because in compounds the atoms are chemically bonded together whereas in a mixture there is no chemical bond

So a mixture can just be separated by physical methods such as distillation

56
Q

What is a mixture

A

When various substances are mixed together w NO CHEMICAL BOND between them

57
Q

Pure substances have a ___ boiling point whereas mixtures….

A

Pure substances have a FIXED boiling point whereas a mixture MAY MELT/ BOIL OVER A RANGE OF TEMPERATURES

58
Q

What is the liquid that has gone thru the filter paper called

A

FILTRATE

59
Q

What is crystallisation used for?

A

Crystallisation is used to separate a solute from a solution

60
Q

Separate a soluble salt from a solution

A

CRYSTALLISATION METHOD

1) pour solution into evaporating basin
2) heat + once H2O has evaporated (u will see crystals start to form as it becomes insoluble) remove dish cos this is the POINT OF CRYSTALLISATION
3) filter the crystals out of the solution + leave to dry (use a DESSICATOR)

61
Q

What is a dessicator

A

It dries things out by removing water from surroundings using chemicals

62
Q

Why is simple distillation more often used than crystallisation at separating a mixture

A

Because in crystallisation the water is lost = a waste

Simple distillation saves the water

63
Q

Why do substances in a mixture separate on a chromatogram ?

A

Because the substances in a mixture have different attractions to the paper or solvent

64
Q

What word is used in chromatography when the ink doesn’t travel far up the chromatogram

A

STATIONARY PHASE

cos the ink doesn’t travel far with the solvent + is attracted to the paper

65
Q

What word is used in chromatography when the ink travels far up the chromatogram

A

MOBILE PHASE

Cos the ink is attracted to the solvent + moves a long way w it

66
Q

Design an experiment to investigate the composition of a dye with paper chromatography

A

1) put different spots of ink using a teat pipette in a line on filter paper
2) draw pencil line below for solvent to go into ( don’t touch ink w/ solvent as it will dissolve in)
3) fill up to the line w solvent (e.g. water)
4) place a lid to stop solvent evaporating
5) the solvent will carry the dyes w it , wait till dry— now mark a line where the solvent goes up to

67
Q

Why might the dots of dye on a chromatogram not move from the pencil line during an experiment… how do we fix it?

A

The dye may be insoluble + therefore u need a different solvent

68
Q

How does one work out the Rf values on a chromatogram ?

A

Rf = distance travelled by sample
——————————————
distance travelled by solvent

(Always measure distance by sample from the MIDDLE of the dot)

69
Q

How does one find a mole of an element? and what is a mole?

A

1 mole of a substance =
RAM/ RFM in GRAMS

A mole is the amount of a substance

70
Q

If the mass number of Sulfur is 32 what is the mass of 1 mole of sulfur

A

1 mole of sulfur = 32 g of sulfur

71
Q

How many atoms are there in a mole

A

6.023 x 10^23 atoms = 1 mole

72
Q

Number of moles =

A

Number of moles = mass
————
RAM

73
Q

Why is % yield not 100%? (Give 3 reasons)

A
  • not all reactants used up
  • products escape the reaction vessel
  • REVERSIBLE reaction
74
Q

What is 1 dm^3 in cm^3

A

1dm^3 = 1000cm^3

75
Q

Explain the difference between a strong acid and a weak acid

A

A strong acid is completely ionised in solution (has a pH of 1-3)

whereas Weak acids are not completely ionised (has a pH of 4-6)

IGCSE Chemistry (4 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions